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I know that ionization energy is the energy needed to remove an electron from an atom. The further away the electron is from the nucleus, the easier it is to remove the electron. Ionization energies decrease down a group and increase across a period.
Ionization energy is the amount of energy required to remove the most loosely bound electron from a neutral atom in the gaseous state, whereas electronegativity is the measure of the tendency of an atom to attract a bonding pair of electrons. Ionization energy increases across a period (more protons in an atom attracts electrons more strongly) and decreases down a group (due to electron shielding and greater atomic radius). Electronegativity has similar trends.
There is not an explicit electronegativity trend because at some point the atoms with more protons (meaning a greater electron affinity) end up having so many electrons that their valence electrons are far away from the nucleus and so their electron affinity and electronegativity decreases. At that point it becomes difficult to determine the exact levels of electronegativity of elements. The main point to know is that elements in the top right of the periodic table tend to be more electronegative.
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